Question

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=> A 6.90 M solution of KOH in water contains 30% by mass of KOH. Calculate the density of KOH Solution (Given= molar mass of 56 g mol^-1).

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Answer 1

${\bold{\underline{\underline{Answer :}}}}$

Solution :

6.90 M solution of KOH contains 6.90 moles

of KOH in 1000 mL of solution

Therefore Wt. of solution in KOH

= 6.90 × 56 = 386.4 g.

Since the solution is 30% by weight, it means that 30 g of KOH are present in 100 g of solution.

$\therefore$386.4 g of KOH is present in

=$\frac{100}{30}\times386.4\:=1288\:g\:of \:solution$

Now, Density = $\frac{Weight}{Volume}$

$\implies$$\frac{1288}{1000} = 1.288 \:mL^{ - 1}$